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A 100 mL solution of 1 M CuSO4 is electrolysed with 0.5A of current until its conc. becomes 0.4 M. If vol. of sol. remains constant, how long electrolysis was conducted?
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A 100 mL solution of 1 M CuSO4 is electrolysed with 0.5A of current un...
Understanding the Electrolysis of CuSO4
Electrolysis involves using an electric current to drive a chemical reaction. In this case, we are electrolyzing a 100 mL solution of 1 M CuSO4.
Initial and Final Concentration
- Initial concentration of CuSO4 = 1 M
- Final concentration after electrolysis = 0.4 M
- Volume of solution = 100 mL
Change in Concentration
- The change in concentration = Initial concentration - Final concentration
- Change = 1 M - 0.4 M = 0.6 M
Volume of CuSO4 Consumed
- Moles of CuSO4 consumed = Change in concentration × Volume (in L)
- Change in concentration = 0.6 M
- Volume = 0.1 L (100 mL)
- Moles consumed = 0.6 × 0.1 = 0.06 moles
Electrolysis and Charge Calculations
- Each mole of CuSO4 requires 2 moles of electrons (2 Faradays) for complete reduction.
- Charge required = Moles consumed × 2 (for Cu2+) × Faraday's constant (approximately 96500 C/mol)
- Charge required = 0.06 moles × 2 × 96500 C/mol = 11580 C
Time Calculation
- Current (I) = 0.5 A
- Time (t) = Charge (Q) / Current (I)
- Time = 11580 C / 0.5 A = 23160 seconds
Conclusion
- The duration of electrolysis was approximately 23160 seconds, or 6 hours and 26 minutes, to reduce the concentration of CuSO4 from 1 M to 0.4 M while keeping the volume constant.
Electrolysis involves using an electric current to drive a chemical reaction. In this case, we are electrolyzing a 100 mL solution of 1 M CuSO4.
Initial and Final Concentration
- Initial concentration of CuSO4 = 1 M
- Final concentration after electrolysis = 0.4 M
- Volume of solution = 100 mL
Change in Concentration
- The change in concentration = Initial concentration - Final concentration
- Change = 1 M - 0.4 M = 0.6 M
Volume of CuSO4 Consumed
- Moles of CuSO4 consumed = Change in concentration × Volume (in L)
- Change in concentration = 0.6 M
- Volume = 0.1 L (100 mL)
- Moles consumed = 0.6 × 0.1 = 0.06 moles
Electrolysis and Charge Calculations
- Each mole of CuSO4 requires 2 moles of electrons (2 Faradays) for complete reduction.
- Charge required = Moles consumed × 2 (for Cu2+) × Faraday's constant (approximately 96500 C/mol)
- Charge required = 0.06 moles × 2 × 96500 C/mol = 11580 C
Time Calculation
- Current (I) = 0.5 A
- Time (t) = Charge (Q) / Current (I)
- Time = 11580 C / 0.5 A = 23160 seconds
Conclusion
- The duration of electrolysis was approximately 23160 seconds, or 6 hours and 26 minutes, to reduce the concentration of CuSO4 from 1 M to 0.4 M while keeping the volume constant.
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A 100 mL solution of 1 M CuSO4 is electrolysed with 0.5A of current un...
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A 100 mL solution of 1 M CuSO4 is electrolysed with 0.5A of current until its conc. becomes 0.4 M. If vol. of sol. remains constant, how long electrolysis was conducted?
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A 100 mL solution of 1 M CuSO4 is electrolysed with 0.5A of current until its conc. becomes 0.4 M. If vol. of sol. remains constant, how long electrolysis was conducted? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about A 100 mL solution of 1 M CuSO4 is electrolysed with 0.5A of current until its conc. becomes 0.4 M. If vol. of sol. remains constant, how long electrolysis was conducted? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A 100 mL solution of 1 M CuSO4 is electrolysed with 0.5A of current until its conc. becomes 0.4 M. If vol. of sol. remains constant, how long electrolysis was conducted?.
A 100 mL solution of 1 M CuSO4 is electrolysed with 0.5A of current until its conc. becomes 0.4 M. If vol. of sol. remains constant, how long electrolysis was conducted? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about A 100 mL solution of 1 M CuSO4 is electrolysed with 0.5A of current until its conc. becomes 0.4 M. If vol. of sol. remains constant, how long electrolysis was conducted? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A 100 mL solution of 1 M CuSO4 is electrolysed with 0.5A of current until its conc. becomes 0.4 M. If vol. of sol. remains constant, how long electrolysis was conducted?.
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